In the specific heat measurement does the sample have to be 100 C, or would a lower initial temperature do just aa well?

I wrote down it doesn't matter, but i don't know why.

I would go for lower, less lost heat to affect calcuations.

Well, it's funny you should ask! When it comes to measuring specific heat, the initial temperature of the sample doesn't have to be 100°C. In fact, you could start with a lower temperature and still get some pretty cool results! See what I did there? *wink*

The important thing is that you heat up the sample and measure how much energy it takes to raise its temperature. So whether you start with a chilly 10°C, a lukewarm 50°C, or a scorching 100°C, the specific heat can still be determined as long as you keep track of the changes in temperature and energy. And let's be honest, who wouldn't enjoy a little temperature change? It's like going from "Netflix and chill" to "Netflix and spill." So the choice is yours, my friend! Just make sure to calculate those sizzling specific heat values correctly.

Remember, in the world of specific heat measurements, temperatures may rise, but the fun never cools down!

In specific heat measurement, it is not necessary for the sample to start at exactly 100°C. A lower initial temperature can also be used.

The specific heat capacity, denoted as "c" or "C," is the amount of heat energy required to raise the temperature of a substance by a certain amount. In most cases, the specific heat capacity is determined under constant pressure conditions.

To measure the specific heat of a substance, the sample is often heated or cooled to a known temperature and then placed in contact with a heat source or sink of a known temperature. The heat transfer between the sample and the heat source/sink is then measured to determine the specific heat capacity.

The important factor in the measurement is the temperature difference (∆T) between the initial and final temperatures of the sample. The specific heat capacity is calculated using the formula:

q = mc∆T

Where:
- q represents the heat transfer
- m is the mass of the sample
- c is the specific heat capacity
- ∆T is the change in temperature

As long as the temperature difference (∆T) is accurately measured, the specific heat capacity can be determined regardless of the initial temperature of the sample. Therefore, a lower initial temperature can be used, provided that the change in temperature (∆T) is accurately measured.

In the measurement of specific heat, it is not necessary for the sample to be at exactly 100°C. Instead, any initial temperature can be used, including a lower temperature. Let me explain why.

The specific heat of a substance is defined as the amount of heat energy required to raise the temperature of a unit mass of the substance by one degree Celsius (or one Kelvin). It is denoted by the symbol "C."

To measure the specific heat of a substance, we typically use the equation:

Q = m * C * ΔT,

where Q represents the heat energy transferred, m represents the mass of the substance, C represents the specific heat, and ΔT represents the change in temperature.

In this equation, you can see that the specific heat (C) is a constant value for a given substance. Therefore, it does not depend on the initial temperature of the substance. Whether the initial temperature is 100°C or lower, the specific heat remains the same.

However, it is worth noting that the accuracy of the measurement can be affected by the temperature difference (ΔT) between the initial and final states. A larger temperature difference generally leads to a more accurate measurement.